Term
| How many quantum numbers are used to describe the properties of electrons in atomic orbitals? |
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| A spherical electron cloud surrounding an atomic nucleus would best represent..... |
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| How many electrons can an energy level of n=4 hold? |
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| How many electrons can an energy level of n=2 hold? |
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| Compared with an electron for which n=2, an electron for which n=4 has more...... |
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Definition
| Every orbital in a sublevel is singly occupied before any orbital is doubly occupied. |
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| What is the Pauli exclusion? |
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Definition
| no two electrons can have the same four electronic quantum numbers. |
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Term
| In the modern periodic table, elements are ordered... |
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Definition
| according to increasing atomic number. |
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Term
| Mendeleev noticed that certain similarities in the chemical properties of elements appeared at regular intervals when the elements were arranged in order of increasing.......... |
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Term
| The modern periodic law states that.... |
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Definition
| the physical and chemical properties of an element are functions of its atomic number. |
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Term
| The discovery of the noble gases changed Mendeleevs periodic table by adding a new... |
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Term
| The most distinctive property of the noble gases is that they are...... |
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Term
| Lithium, the first element in Group 1, has an atomic number of 3. The second element in this group has an atomic number of.... |
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An isotope of fluorine has a mass number of 19 and an atomic number of 9.
a.How many protons are in this atom?
b.How many neutrons are in this atoms?
c.What is symbol of this atom,and mass number? |
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Term
Samarium, Sm is a member of the lanthanide series.
a. Identify the element just below samarium in the periodic table.
b. By how many units do the atomic numbers of these two elements differ? |
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A certain isotope contains 53 protons, 78 neutrons, and 54 electrons.
a. What is its atomic number?
b. What is the mass number of this atom?
c. What is the name of this element? |
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Definition
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Term
| In a modern periodic table, every element is a member of both a horizontal row and a vertical column. Which one is the group, and which one is the period? |
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Definition
| A period is a horizontal, and a group is vertical. |
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Term
| Explain the distinction between atomic mass and atomic number of an element. |
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Definition
| The atomic number is the number of protons in an atom. The atomic mass is a weighted average of the masses of the naturally occurring isotopes of that element. |
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Term
Give the group numbers that make up each of the following blocks:
a. s block
b. p block
c. d block |
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Term
| When an electron is added to a neutral atom, energy is.. |
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Definition
| either absorbed or released. |
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Term
| The energy required to remove an electron from a neutral atom is the atom's.... |
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Definition
| neither absorbed nor released. |
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Term
From left to right across a period on the periodic table,
a. electron affinity values tend to become more (negative or positive)
b. ionization energy values tend to (increase or decrease)
c. atomic radii tend to become (larger or smaller)
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Definition
a. negative
b. increase
c. smaller |
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Term
| Name the halogen with the least-negative electron affinity. |
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Definition
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Term
| Name the alkali metal with the highest ionization energy. |
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Definition
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| Name the element in period 3 with the smallest atomic radius. |
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Term
| Name the group 14 element with the largest electronegativity. |
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Definition
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Term
| Compare the radius of a positive ion to the radius of its neutral atom. |
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Definition
| The radius of a positive ion is smaller than the radius of its corresponding neutral atom. |
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Term
| Compare the radius of a negative ion to the radius of its neutral atom. |
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Definition
| The radius of a negative ion is larger than the radius of the corresponding neutral atom. |
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Term
| Where are metals, and nonmetals on the periodic table? |
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Definition
| Metals are found on the left side of the periodic table, mostly in the s,d, and f blocks. Nonmetals are on the right side of the periodic table, found in all of the p block (except for hydrogen) |
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Term
| Explain why the second ionization energy is higher than the first, the third is higher than the second, and so on. |
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Definition
| As electrons are removed in successive ionizations, fewer electrons remain within the atom to shield the attractive force of the nucleus. each electron removed from an ion experiences a stronger effective nuclear pull than the electron removed before it. |
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Term
| Explain the role of valence electrons in the formation of chemical compounds. |
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Definition
| Valence electrons most subject to the influence of nearby atoms or ions. They are the electrons available to be lost, gained, or shared in the formation of chemical compounds. |
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Term
| In which block are metalloids found? |
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Definition
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Term
| In which block are the hardest, most densest metals found? |
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Definition
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Term
| Name the most chemically active halogen. |
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Definition
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Term
| Which has a larger radius Al or In? |
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Definition
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Term
| Which class has greater ionization energies, metals or nonmetals? |
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Definition
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Term
| An elements with a large negative electron affinity is most likely to form a ... |
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Definition
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Term
| Which has a stronger electron attraction, a large atom or small atom? |
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